Electronegativity Test Flashcards
1
Q
what properties can categorize substances?
A
conductivity and dissolving
2
Q
a substance that does dissolve in water
A
soluble
3
Q
substance that does not dissolve in water
A
insoluble
4
Q
conductivity
A
a property that describes how well a substance transmits electricity, heat, or sound
5
Q
what does electrical conductivity require?
A
the movement of charge as ions or electrons
6
Q
in the body how does electricity move?
A
as ions, not as electrons
7
Q
how can conductivity be tested?
A
by setting up an electrical circuit. the wires connect to a battery, the substance, and a light bulb, if the light bulb turns on, it is conductive
8
Q
substance that dissolves and conducts
A
Ionic, metal and nonmetal atoms
9
Q
substance that dissolves and doesn’t conduct
A
molecular covalent, nonmetal atoms only (carbon, hydrogen, oxygen)
10
Q
substance that doesn’t dissolve and conducts
A
metallic, metal atoms only
11
Q
substance that doesn’t dissolve and doesn’t conduct
A
network covalent, nonmetal atoms only
12
Q
only substances that contain___ atoms will conduct electricity
A
Metal
13
Q
substances made entirely out of ___ atoms will not dissolve in water
A
Metal
14
Q
Many ___ compounds dissolve in water
A
Ionic
15
Q
what is a chemical bond?
A
the bond that hold atoms together, is the attraction of positive charges in the nucleus and negative charges in the electrons of another atom
16
Q
Ionic bonding
A
- Dissolve in water
- conduct when dissolved
- tend to be brittle solids
- made of metal and non metals
17
Q
Molecular Covalent Bonding
A
- Some dissolve in water
- do no conduct
- some are liquids or gases
- made entirely of non metal atoms
18
Q
Metallic Bonding
A
- Don’t dissolve
- conducts
- bendable/ malleable solids
- made entirely of metal atoms
19
Q
Network Covalent
A
- Do not dissolve in water
- Do not conduct electricity
- Extremely hard solids
- Made entirely of non metal atoms
20
Q
Covalent Bonding
A
- the nucleus of one atom is attracted to the valence electrons of another atom.
- one atom doesn’t transfer an electron to the other. both atoms share the valence electron.
21
Q
in molecular covalent, what do the atoms bond into
A
forms into individual clusters called molecules
22
Q
in network covalent bonding, how are the valence electrons shared
A
valence electrons are shared between atoms, but form a highly regular extended network, creating a very durable structure
23
Q
in metallic bonding, the electrons are ___
A
- distributed around the substance in what is called a sea of electrons.
- the valence electrons are free to move throughout the substance.
- they are bonded by the attraction between positively charged atoms and negatively charged “sea” of electrons.
24
Q
what does conduction require?
A
the movement of a charged particle (ion or electron)
25
why do metal conduct?
the valence electrons can freely move throughout the solid
26
why do ionic compounds that dissolve conduct
because the cations and anions move freely in the solution
27
why do network covalent solids and molecular covalent substances do not conduct
the electrons are stuck between the atoms and are not available to move, so the charge cannot move.
28
polar molecules are ___ to a charged wand, and ___ smell
attracted, Do smell
29
nonpolar molecules are__ to a charged wand, and __ smell
no attracted, Don't smell
30
Partial charge
smaller than the charge on an individual electron or proton
31
when a negative charged wand is next to water, why does it pull towards the water?
the molecules in the water orient themselves so that positive is in the direction of the wand, attracting the stream to the wand
32
intermolecular force
the attraction between individual molecules in a substance
33
why does water bead up?
because it is polar, so they attract to each other
34
why does oil spread out
it is nonpolar, they are not attracted to each other, and spread out
35
why is water a liquid and methane a gas at room temperature
water is polar, methane is nonpolar. the individual water molecules are attracted to each other and stay as a liquid, the methane attractions are weaker, which means they spread out easier.
36
Methanol dissolves in water, oil does not
polar methanol attracts to the polar water molecules. the non polar oil does not attract well with the polar water molecules
37
non polar covalent bonds
bonds with the same negativity value
38
polar covalent bonds
share electrons unequally, more attracted to one atom (partial)
39
Ionic bonds
A large difference in electronegativity, more electronegative ion takes the electrons and becomes a negative ion, the other becomes positive
40
what bonds create dipoles?
polar bonds
41
what is a dipole?
the polarity of an individual bond between atoms
42
what other properties does polarity effect in a molecule?
solubility, smell, boiling and melting points
43
electronegativity
the tendency of an atom to attract shared electrons
44
why is a polar molecule called a dipole?
because it has 2 poles (+ and - ends)
45
atoms that are more electronegative end up having ____
a partial negative charge
46
when is a molecule non polar
when 2 atoms with identical electronegativities bond together
47
since CO_2 has 2 dipoles, why isn't it a polar molecule?
the 2 dipoles balance each other, there is no partial positive end to the molecule
48
when 2 atoms with different electronegativities bond together, what is the result? why
a polar covalent bond/ because there is a partial negative charge
49
when 2 atoms have identical electronegativities, what is the result? why
nonpolar covalent/ there is no partial charge
50
if there is a big difference in the electronegativities of 2 atoms, what is the result? why
Ionic bond/ the electronegative pull is so great that it is possible for the electrons to be pulled entirely towards one of the atoms in a bond
51
who proposed the scale for electronegativity
Linus Pauling, in 1932
52
what does the electronegativity scale allow you to do?
- compare individual atoms electronegativity/
| - the polarity of bonds
53
diatomic molecules
molecules with 2 atoms
54
how do you compare the polarity of one bond to another?
by looking at the numerical difference between the electronegativities of the 2 atoms
55
bond with a bigger difference in electronegativity between the 2 atoms are_____
more polar
56
when the difference between electronegativity between 2 atoms is very large, the bond is considered ___
it is no longer considered covalent
57
when 2 atoms are no longer considered covalent, the electrons are transferred from ___ to ____.
the less electronegative atom to the more electronegative atom.
58
after the electrons are transfered from one atom to another what forms and what is then created?
A cation and anion form and are attracted to one another and then create an ionic bond
59
chemical bond
an attraction between atoms that holds them together
60
covalent bonding
type of chemical bonding in which 1 or more pairs of valence electrons are shared between the atoms
61
structoral formula
OH CH_2 CH_2 CH_2 OH
62
molecular formula
C_3 H_8 O_2
63
HONC
1234 rule, draw carbon first, then nitrogen, then oxygen, then hydrogen
64
bonded pair
pair of electrons that are shared in a covalent bond between 2 atoms
65
lone pair
pair of unshared valence electrons that are not involved in bonding in a molecule
66
octet rule
non metals combine by sharing electrons so that each atom has a total of eight valence electrons. after bonding, each atom resembles a noble gas in its electron arrangement (8 electrons)
67
diatomic molecule
a molecule consisting of 2 atoms
68
how to name an ionic compound
METAL AND NON METAL
- always name cation first (metal) then anion (nonmetal)
- the cation always stay the same
- the anion takes the root of the word and then adds "-ide" to the end
ex: Calcium SulfIDE (CaS)
69
how to name a polyatomic ion
SAME AS IONIC EXCEPT:
-the anion name is found on the common ion sheet
-if there are multiple anions, use parenthesis in the formula, to show the polyatomic anion as a single unit, followed by a subscript number
ex: NaNO_3= Sodium Nitrate
MgSO_4 Magnesium Sulfate
(NO "-IDE" IS NEEDED)
70
How to name transition metal cations
- the name of the compound includes a roman numeral to indicate which ion is in the compound
- the charge of the cation can be determined from the formula by balancing the charge of the anion to give a net charge of zero
ex: FeO iron(ii) oxide
71
Naming covalent compounds
ONLY NONMETALS
-the first element in the formula is named first, and the full element name is used
-the second element is named as though it was an anion
-a prefix is used before the second element, to denote the number of atoms present
-never use mono for the first element
ex: CO_2 carbon monoxide
N_2O_5 dinitrogen pentaoxide
P_4O_6 tetraphosphorus hexoxide
72
Naming Acids
```
ALWAYS HAVE H IN THEM (except for acetic acid)
- use polyatomic ions to name acids
ex: HCLO_4 Percloric acid
HNO_3 Hydronitric acid
HCL Hydrocloric acid
HBr Hydrobromic acid
H_3PO_4 hydrogen phosphuric acid
HCLO_2 Hydro Clourous acid
HCLO_3 chloric acid
```
